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{{chembox |
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| verifiedrevid = 400325686 |
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| Watchedfields = changed |
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| Name = Nickel(II) hydroxide |
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| verifiedrevid = 437323024 |
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| ImageFile = Hydroxid nikelnatý.PNG |
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| ImageName = Nickel(II) hydroxide |
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| Name = Nickel(II) hydroxide |
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| ImageFile1 = Hydroxid nikelnatý.PNG |
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| IUPACName = |
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| ImageName1 = Nickel(II) hydroxide |
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| OtherNames = |
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| ImageFile2 = Kristallstruktur Cadmiumiodid.png |
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| Section1 = {{Chembox Identifiers |
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| ImageName2 = Nickel(II) hydroxide |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| IUPACName = Nickel(II) hydroxide |
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| OtherNames = Nickel hydroxide, Theophrastite |
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|Section1={{Chembox Identifiers |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 55452 |
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| ChemSpiderID = 55452 |
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| PubChem = 61534 |
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| PubChem = 61534 |
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| StdInChIKey = BFDHFSHZJLFAMC-UHFFFAOYSA-L |
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| StdInChIKey = BFDHFSHZJLFAMC-UHFFFAOYSA-L |
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| CASNo = 12054-48-7 |
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| CASNo = 12054-48-7 |
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| CASNo_Ref = {{cascite|??|??}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo2_Ref = {{cascite|changed|??}} |
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| CASOther = <br/>36897-37-7 (monohydrate) |
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| EINECS = |
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| CASNo2 = 36897-37-7 |
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| CASNo2_Comment = (monohydrate) |
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| RTECS = QR6480000 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = L8UW92NW6J |
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| EINECS = 235-008-5 |
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| RTECS = QR648000 |
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| Section2 = {{Chembox Properties |
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|Section2={{Chembox Properties |
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| Formula = Ni(OH)<sub>2</sub> |
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| Formula = Ni(OH)<sub>2</sub> |
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| Appearance = green crystals |
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| Appearance = green crystals |
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| Density = 4.10 g/cm<sup>3</sup> |
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| Density = 4.10 g/cm<sup>3</sup> |
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| MolarMass = 92.708 g/mol (anhydrous) <br> 110.72 g/mol (monohydrate) |
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| MolarMass = 92.724 g/mol (anhydrous) <br> 110.72 g/mol (monohydrate) |
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| Solubility = 0.0015 g/L<ref>{{cite book|isbn=0849304849|title=CRC Handbook of Chemistry and Physics|edition=84|pages=4–71|year=2003|publisher=CRC press}}</ref> |
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| Solubility = insoluble |
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| SolubilityProduct = 5.48{{e|−16}}<ref name="crc">{{cite book |author1=John Rumble |title=CRC Handbook of Chemistry and Physics |date=June 18, 2018 |publisher=CRC Press |isbn=978-1138561632 |pages=5–189|edition=99 |language=English}}</ref> |
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| SolubleOther = soluble in dilute ], ] (monohydrate) |
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| MeltingPtC = 230 |
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| MeltingPt = 230 °C (anhydrous, decomp) |
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| MeltingPt_notes = (anhydrous, decomposes) |
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| MagSus = +4500.0·10<sup>−6</sup> cm<sup>3</sup>/mol |
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| Section3 = {{Chembox Structure |
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|Section3={{Chembox Structure |
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| Structure_ref =<ref>{{cite journal|doi=10.1143/JPSJ.39.317|title=Magnetic Behaviours of a Random Magnet, Ni<sub>p</sub>Mg<sub>(1-p)</sub>(OH<sub>2</sub>)|journal=Journal of the Physical Society of Japan|volume=39|issue=2|pages=317|year=1975|last1=Enoki|first1=Toshiaki|last2=Tsujikawa|first2=Ikuji|bibcode=1975JPSJ...39..317E}}</ref> |
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| Coordination = |
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| CrystalStruct = hexagonal |
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| CrystalStruct = hexagonal, ] |
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| SpaceGroup = P{{overline|3}}m1, No. 164 |
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| LattConst_a = 0.3117 nm |
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| LattConst_b = 0.3117 nm |
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| LattConst_c = 0.4595 nm |
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| LattConst_alpha = 90 |
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| LattConst_beta = 90 |
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| LattConst_gamma = 120 |
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| LattConst_ref = |
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| Coordination = |
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| Dipole = |
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| Section4 = {{Chembox Thermochemistry |
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|Section4={{Chembox Thermochemistry |
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| DeltaHf = −538 kJ·mol<sup>−1</sup><ref name=b1>{{cite book| author = Zumdahl, Steven S.|title =Chemical Principles |edition=6| publisher = Houghton Mifflin Company| year = 2009| isbn = 978-0-618-94690-7|page=A22}}</ref> |
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| DeltaHf = -530.049 kJ/mol |
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| Entropy = 79 J·mol<sup>−1</sup>·K<sup>−1</sup><ref name=b1/> |
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| Section7 = {{Chembox Hazards |
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|Section7={{Chembox Hazards |
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| ExternalMSDS = |
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| ExternalSDS = |
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| EUClass = |
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| GHSPictograms = {{GHS07}}{{GHS08}} |
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| EUIndex = |
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| GHS_ref = <ref name="sds">{{cite web|title = Nickel Hydroxide|url = https://www.americanelements.com/nickel-hydroxide-12054-48-7|publisher = ]|access-date = 2018-08-30}}</ref> |
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| GHSSignalWord = Danger |
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| HPhrases = {{H-phrases|302|332|315|334|317|341|350|360|372}} |
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| PPhrases = {{P-phrases|260|284|201|280|405|501}} |
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| NFPA-H = |
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| NFPA-H = |
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| NFPA-F = |
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| NFPA-F = |
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| NFPA-R = |
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| NFPA-R = |
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| NFPA-O = |
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| NFPA-S = |
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| RPhrases = |
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| SPhrases = |
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| FlashPt = |
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| FlashPt = |
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| LD50 = 1515 mg/kg (oral, rat) |
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| Section8 = {{Chembox Related |
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|Section8={{Chembox Related |
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| OtherAnions = |
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| OtherAnions = |
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| OtherCations = |
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| OtherCations = |
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| OtherCompounds = |
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'''Nickel(II) hydroxide''' is the ] with the formula Ni(OH)<sub>2</sub>. It is a lime-green solid that dissolves with decomposition in ] and ] and is attacked by acids. It is electroactive, being converted to the ], leading to widespread applications in ].<ref name="Chen">{{cite journal|author1=Chen, J. |author2=Bradhurst, D.H. |author3=Dou, S.X. |author4=Liu, H.K. |title= Nickel Hydroxide as an Active Material for the Positive Electrode in Rechargeable Alkaline Batteries |doi= 10.1149/1.1392522 |journal=Journal of the Electrochemical Society |year=1999|volume= 146|issue= 10 |pages=3606–3612|bibcode=1999JElS..146.3606C |s2cid=33058220 |url=https://ro.uow.edu.au/cgi/viewcontent.cgi?article=1118&context=engpapers }}</ref> |
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'''Nickel(II) hydroxide''' Ni(OH)<sub>2</sub> is an ] ] commonly used in ] electrodes. When charged these electrodes form ]. Nickel(II) hydroxide is a precipitate formed when the hexaaquanickel(II) ion is mixed with aqueous alkali. The mineralogical form is very rare and is called theophrastite. |
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==Properties== |
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Nickel(II) hydroxide has two well-characterized ]s, α and β. The α structure consists of Ni(OH)<sub>2</sub> layers with intercalated anions or water.<ref name=Oliva>{{cite journal|author1=Oliva, P. |author2=Leonardi, J. |author3=Laurent, J.F. |title=Review of the structure and the electrochemistry of nickel hydroxides and oxy-hydroxides|journal=Journal of Power Sources|year=1982|doi=10.1016/0378-7753(82)80057-8| volume =8|issue=2|pages= 229–255|bibcode=1982JPS.....8..229O }}</ref><ref name=Jeevandam>{{cite journal|author1=Jeevanandam, P. |author2=Koltypin, Y. |author3=Gedanken, A. |title= Synthesis of Nanosized α-Nickel Hydroxide by a Sonochemical Method|journal= Nano Letters|doi=10.1021/nl010003p|year= 2001|volume= 1|issue= 5|pages= 263–266|bibcode=2001NanoL...1..263J }}</ref> The β form adopts a ] of Ni<sup>2+</sup> and OH<sup>−</sup> ions.<ref name=Oliva/><ref name=Jeevandam/> In the presence of water, the α polymorph typically recrystallizes to the β form.<ref name=Oliva/><ref name=Shukla>{{cite journal|author1=Shukla, A.K. |author2=Kumar, V.G. |author3=Munichandriah, N. |title= Stabilized α-Ni(OH)<sub>2</sub> as Electrode Material for Alkaline Secondary Cells |journal= Journal of the Electrochemical Society |year=1994|volume= 141|issue= 11 |pages= 2956–2959|doi= 10.1149/1.2059264 |bibcode=1994JElS..141.2956V }}</ref> In addition to the α and β polymorphs, several γ nickel hydroxides have been described, distinguished by crystal structures with much larger inter-sheet distances.<ref name=Oliva/> |
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The mineral form of Ni(OH)<sub>2</sub>, ], was first identified in the Vermion region of northern Greece, in 1980. It is found naturally as a translucent emerald-green crystal formed in thin sheets near the boundaries of idocrase or chlorite crystals.<ref name=Marcopoulos>{{cite journal|author1=Marcopoulos, T. |author2=Economou, M. |journal=American Mineralogist|year= 1980|volume= 66|pages= 1020–1021|url=http://www.minsocam.org/ammin/AM66/AM66_1020.pdf|title=Theophrastite, Ni(OH)<sub>2</sub>, a new mineral from northern Greece }}</ref> A nickel-magnesium variant of the mineral, {{chem2|(Ni,Mg)(OH)2}} had been previously discovered at Hagdale on the island of ] in Scotland.<ref>{{cite journal|author1=Livingston, A. |author2=Bish, D. L. |year=1982|title=On the new mineral theophrastite, a nickel hydroxide, from Unst, Shetland, Scotland|page=1|url=http://www.minersoc.org/pages/Archive-MM/Volume_46/46-338-1.pdf|journal=Mineralogical Magazine|volume=46|issue=338|doi=10.1180/minmag.1982.046.338.01|bibcode=1982MinM...46....1L |s2cid=8381523 }}</ref> |
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==Reactions== |
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Nickel(II) hydroxide is frequently used in electrical car batteries.<ref name=Jeevandam/> Specifically, Ni(OH)<sub>2</sub> readily oxidizes to nickel oxyhydroxide, NiOOH, in combination with a reduction reaction, often of a metal hydride (reaction 1 and 2).<ref name=Ovshinsky>{{cite journal|author1=Ovshinsky, S.R. |author2=Fetcenko, M.A. |author3=Ross, J. |title=A nickel metal hydride battery for electric vehicles|journal=Science|year= 1993|volume= 260|issue=5105|pages= 176–181|pmid=17807176|doi=10.1126/science.260.5105.176|bibcode=1993Sci...260..176O |s2cid=9523468 }}</ref><ref>{{Cite book|last=Young|first=Kwo|url=https://www.mdpi.com/books/pdfview/book/244|title=Nickel Metal Hydride Batteries|publisher=MDPI|year=2016|isbn=978-3-03842-303-4|language=en|doi=10.3390/books978-3-03842-303-4|doi-access=free}}</ref> |
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'''Reaction 1''' |
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{{chem2|Ni(OH)2 + OH(–) → NiO(OH) + H2O + e(−)}} |
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'''Reaction 2''' |
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{{chem2|M + H2O + e(−) → MH + OH(−)}} |
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'''Net Reaction''' (in H<sub>2</sub>O) |
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{{chem2|Ni(OH)2 + M → NiOOH + MH}} |
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Of the two polymorphs, α-Ni(OH)<sub>2</sub> has a higher theoretical capacity and thus is generally considered to be preferable in electrochemical applications. However, it transforms to β-Ni(OH)<sub>2</sub> in alkaline solutions, leading to many investigations into the possibility of stabilized α-Ni(OH)<sub>2</sub> electrodes for industrial applications.<ref name=Shukla/> |
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==Synthesis== |
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The synthesis entails treating aqueous solutions of nickel(II) salts with potassium hydroxide. When the same reaction is conducted in the presence of bromine, the product is {{chem2|Ni3O2(OH)4}}.<ref>{{cite book|author1=O. Glemser|chapter=Nickel (II) Hydroxide and Nickel (II,III) Hydroxide|title=Handbook of Preparative Inorganic Chemistry, 2nd Ed. |editor=G. Brauer|publisher=Academic Press|year=1963|place=New York|volume=2|page=1549-1551}}</ref> |
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==Toxicity== |
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The Ni<sup>2+</sup> ion is a carcinogen when inhaled. |
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==See also== |
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==See also== |
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==External links== |
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==References== |
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{{reflist}} |
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{{Nickel compounds}} |
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{{Nickel compounds}} |
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{{Hydroxides}} |
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{{inorganic-compound-stub}} |
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